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Aleks [24]
3 years ago
7

Suppose you held two magnets a short distance apart,then let go. what would happen?

Chemistry
2 answers:
Murljashka [212]3 years ago
4 0
The two magnets ought to join together given that at least, if not both, have a strong enough magnetic force to do so.
Assoli18 [71]3 years ago
4 0

Answer:

There are two possibilities that would occur:

  1. The magnets come together and stick together.
  2. The magnets are further apart than the distance at which they were held.

Explanation:

The magnets have two poles: positive and negative, before which it is recognized that <u>if two magnets with the same pole are close to each other and are released, these magnets will repel each other</u>, this is because the same pole repels, regardless of whether it is negative or positive, on the contrary, <u>if the two magnets are close and have opposite poles directed towards each other, these magnets will attract</u>, even with this there is usually a saying that "the opposite poles attract," although it is usually use in couple relationships, this saying may allow you to remember this rule.

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2.93 mol of MgF2 to grams
mojhsa [17]

The mass of 1.72 mol of magnesium fluoride is 107 grams.

To determine the mass of 1.72 mol of magnesium fluoride, we first need the chemical formula of magnesium fluoride. Magnesium forms a +2 ion (Mg+2) and fluoride forms a -1 ion (F-1). Since all compounds formed from ions have to be electrically neutral, we need 2 fluoride ions and 1 magnesium ion. Therefore, the formula for magnesium fluoride is MgF2.

Now we need to determine the molar mass of the compound from the molar mass values from the periodic table. Let's use a table to calculate this molar mass.

Molar mass of MgF2

Element Molar Mass (g/mol) Quantity Total (g/mol)

Mg 24.31 1 24.31

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Total molar mass of MgF2 = 24.31 g/mol + 38.00 g/mol = 62.31 g/mol

This is the mass of one mole of the substance. If we have 1.72 mols of it, we multiply 1.72 by 62.31.

1.72 mol (62.31 g/mol) = 107 grams

We rounded to 107 to keep the correct number of significant digits in our answer.

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